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2. Ammonia is synthesized via the following chemical reaction: N2 (9) + 3 H2 (9) 2 2 NH3 (g) Ke = 6.01 x 10-2 For each of the following initial conditions, determine if the given concentrations represent an equilibrium. If not, predict the direction in which the reaction will proceed to reach equilibrium. a. [NH3] = 1.00 x 10-3 mol/L, [N2] = 1.00 x 10-5 mol/L, [H2] = 2.00 x 103 mol/L b. [NH3] = 2.00 x 104 mol/L, [N2] = 1.50 x 10-5 mol/L, [H2] = 3.54 x 10-1 mol/L

2. Ammonia is synthesized via the following chemical reaction: N2 (9) + 3 H2 (9) 2 2 NH3 (g) Ke = 6.01 x 10-2 For each of the following initial conditions, determine if the given concentrations represent an equilibrium. If not, predict the direction in which the reaction will proceed to reach equilibrium. a. [NH3] = 1.00 x 10-3 mol/L, [N2] = 1.00 x 10-5 mol/L, [H2] = 2.00 x 103 mol/L b. [NH3] = 2.00 x 104 mol/L, [N2] = 1.50 x 10-5 mol/L, [H2] = 3.54 x 10-1 mol/L

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 38GQ: At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g)...
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2. Ammonia is synthesized via the following chemical reaction: N2 (g) + 3 H2 (g) 2 2 NH3 (g) Ke = 6.01 x 102 For each of the following initial conditions, determine if the given concentrations represent an equilibrium. If not, predict the direction in which the reaction will proceed to reach equilibrium. a. [NH3] = 1.00 x 10-3 mol/L, [N2] = 1.00 x 10-5 mol/L, [H2] = 2.00 x 103 mol/L b. [NH3] = 2.00 x 104 mol/L, [N2] = 1.50 x 10-5 mol/L, [H2] = 3.54 x 10-1 mol/L %D
Transcribed Image Text:2. Ammonia is synthesized via the following chemical reaction: N2 (g) + 3 H2 (g) 2 2 NH3 (g) Ke = 6.01 x 102 For each of the following initial conditions, determine if the given concentrations represent an equilibrium. If not, predict the direction in which the reaction will proceed to reach equilibrium. a. [NH3] = 1.00 x 10-3 mol/L, [N2] = 1.00 x 10-5 mol/L, [H2] = 2.00 x 103 mol/L b. [NH3] = 2.00 x 104 mol/L, [N2] = 1.50 x 10-5 mol/L, [H2] = 3.54 x 10-1 mol/L %D
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